Question

The concentrated sulpuric acid that si peddled commerical si 95%H2so4 by weight if the Density of this commercial acid is 1.834g cm3 the molarity of this solution is

Answer 1

The molarity of sulphuric acid is 17.8 moles per liter

Explanation:

• Molarity is defined as moles over volume = M = n/V

• Here we are provided with the density e.g. 1.834g/cm-3 or we can say 1.834 g/ml

• We need to covert it to liter to make it consistent with the formula e.g. 1834 g/l

• Now we need to find out the number of mole of sulphuric acid e.g. moles = mass/molar mass

• Moles =n= 1834*0.95/98 = 17.8 moles ( because sulphuric acid is 95% by mass)

• Molarity = M = n/V = 17.8 moles/ liter

Learn more about molarity from the link below

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